1 Chapter 4: Atomic Theory Atom
Compound
Chemical changes
Smallest particle of an
element
A pure substance made from
two or more atoms
Changes in the way atoms and
molecules are arranged
Subatomic particles
Particles that make up an
atom
Proton – what is its charge,
mass and where is it found?
Positive (+1), mass = 1 and
found in the nucleus of an
atom
2 Chapter 4: Atomic Theory Neutron – what is its charge,
mass and where is it found?
No charge (0), mass = 1 and in
the nucleus of an atom
Electron – what is its charge,
mass and where is it found?
Negative charge (-1), mass =
0 and fund circling the
nucleus of an atom
Nuclear charge
The charge of the nucleus of
an atom *count the number
of protons*
Atomic number
Number of protons in the
nucleus of an atom  this
tells us what the element is
Neutral atom
When # protons = #
electrons in an atom
3 Chapter 4: Atomic Theory Period
The row across the periodic
table
Group or family
A column in a periodic table –
have similar chemical
properties
Alkali metals (group 1)
Very reactive metals
Alkaline earth metals (group
2)
Somewhat reactive metals
Halogens (group 17)
Very reactive non-metals
4 Chapter 4: Atomic Theory Noble gases (group 18)
Very unreactive gaseous nonmetals
Transition metals
(groups 3 – 12)
Ions
Formed when atoms gain or
lose electrons
Multivalent
These metals can form more than
one type of ion (ex: Fe3+ and Fe2+)
Cation
Positively charged ion
5 Chapter 4: Atomic Theory Anion
Negatively charged ion
This is:
Bohr diagram
Stable octet
Valence shell
Valence electron
When there are 8 electrons
in outermost shell of an atom
The outermost shell of an
atom that has electrons
An electron that is in the
outer shell (these are the
ones that can be donated)
6 Chapter 4: Atomic Theory Ionic bonding
When one or more electrons
is transferred from a metal
atom to a non-metal atom to
forcompounds
Covalent bonding
When electrons are shared
between non-metal atoms to
form compounds
This is a:
Lewis diagram – it only shows
the electrons in the valence
shell
Diatomic molecules
Pair of atoms joined by
covalent bonds  F2, Br2, H2,
N2, O2, Cl2 and I2
List the rules for naming an
ionic compound
Metal named first
Non-metal second
Change ending to “ide”
7 Chapter 4: Atomic Theory What must you add when
naming an ionic compound
with a multivalent metal?
A Roman numeral to show the
ion charge of the metal being
used
Name:
Zinc iodide
ZnI2
(simple ionic compound)
Name:
NiCl2
What is the formula for?
Strontium nitride
What is the formula for?
Lead (IV) sulphide
Nickel (II) chloride
(multivalent metal)
Sr3N2
(simple ionic compound)
PbS2
(multivalent metal)
8 Chapter 4: Atomic Theory Polyatomic ions
An ion composed of more
than one type of atom (ex:
hydroxide  OH-)
What 2 things must you
remember when writing the
formulas of compounds made
with polyatomic ions?
Brackets if there is more
than one set needed
Do not change the ending of
the name
Where is phosphorous
stored?
Trapped in phosphate that
makes up phosphate rock and
sediments
How do you name binary
covalent compounds?
Name the left element first
Name the second element and
change the ending to “ide”
Add a prefix to each name to
show the number of each atom
Name this:
KCH3COO
Potassium acetate
(polyatomic ions)
9 Chapter 4: Atomic Theory Give the formula for:
KMnO4
Potassium permanganate
(polyatomic ions)
Name this:
Carbon tetrachloride
CCl4
(binary covalent compound)
Give the formula for:
Tetraphosphorous decaoxide
Reactants
Products
P4O10
(binary covalent compound)
Substances mixed to create a
chemical reaction
What is created in a chemical
reaction
10 Chapter 4: Atomic Theory What is the Law of
Conservation of Mass?
The total mass of the
reactants always = the total
mass of the products
This is called:
Methane + oxygen  water + carbon dioxide
Word equation
This is called:
K + O2  K2O
Skeleton equation
This is called:
4K + O2  2K2O
Coefficient
Balanced equation
The number placed in front of a
compound in a balanced equation
to show how many molecules react
or are produced